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Year 9 WCC Exam Revision > Science - Chemistry > Flashcards

Science - Chemistry Flashcards

1
Q

Characteristics of Metals

A
  • Malleable
  • Ductile
  • Lustrous
  • Good conductor of heat
  • Good conductor of electricity
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2
Q

Characteristics of Non-Metals

A
  • Brittle
  • Dull
  • Poor conductor of heat
  • Poor conductor of electricity
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3
Q

Characteristics of Metalloids

A
  • Brittle
  • Lustrous
  • Semiconductors of electricity
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4
Q

An element is a:

A

A substance that is made of only one type of atom

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5
Q

A compound is a:

A

A substance that is made of two or more different elements bonded together

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6
Q

An atom is a:

A

The smallest part of an element

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7
Q

A molecule is a:

A

Two or more atoms bonded together

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8
Q

A lattice is a:

A

An ongoing repeating pattern of atoms bonded together

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9
Q

A mixture is:

A

Two or more elements that are not bonded together, can be seperated

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10
Q

A solution is a:

A

A solute dissolved in a solvent (e.g. salt(solute) dissolved in water(solvent))

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11
Q

An alloy is:

A

A metal mixed with another substance

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12
Q

The big number before a chemical formula means:

A

The quantity of that molecule

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13
Q

Physical change

A

When the molecules don’t change and the bonds do not break. No new molecules are formed.

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14
Q

Chemical change

A

When the molecules have their bond broken and may reform with other atoms, forming new substances. The atoms are rearranged.

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15
Q

A proton has a charge of

A

+1

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16
Q

A neutron has a charge of

A

0 (neutral)

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17
Q

An electron has a charge of

A

-1

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18
Q

A proton has a relative mass of

A

1

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19
Q

A neutron has a relative mass of

A

1

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20
Q

An electron has a relative mass of

A

(negligible),0

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21
Q

Which particles make up the nucleus

A

Protons and Neutrons

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22
Q

Which particles make up the shells

A

Electrons

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23
Q

The atomic number is the _____ number on the periodic table

A

Numerically smaller

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24
Q

The Atomic mass is the ____ number on the periodic table

A

Numerically larger

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25
Q

How do you find the number of Protons an element has？

A

You look at the atomic number

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26
Q

How do you find the amount of neutrons an element has?

A

You take the atomic mass and subtract the atomic number from it

27
Q

How do you find the amount of electrons an element has?

A

For an atom, its the same as the protons

28
Q

Why do some atomic symbols use letters that don’t match up with their names?

A

Because the symbols are derived from other languages

29
Q

Where are metals located on the periodic table?

A

Left of the dividing line

30
Q

Where are non-metals located on the periodic table?

A

Right of the dividing line

31
Q

Where are the metalloids located on the periodic table?

A

On either side of the dividing line

32
Q

A group on the periodic table is a:

A

Column

33
Q

A period on the periodic table is a:

A

Row

34
Q

What is an isotope?

A

An atom with extra, less, or the same neutrons than normal

35
Q

An isotype is written as:

A

(Element name)-(atomic mass)(eg carbon-15)

36
Q

Unstable atoms emit ____ and ____ over time

A

Radiation and decay

37
Q

Changing the amount of electrons an atom has results in a differed ____

A

Ion

38
Q

Capacity of the first 4 electron shells:

A

2,8,8,18

39
Q

Valence electrons are electrons in the ______

A

Outermost/Valence shell

40
Q

The Valence shell is the _____shell

A

Outermost

41
Q

How do you write an electron configuration

A

(Shell 1),(Shell 2),(Shell 3)(etc…)

42
Q

How do you find the charge of an ion using the periodic table

A

Count how many electrons it needs to lose/gain to achieve a full valence shell.

43
Q

A cation

A

A positively charged Ion

44
Q

An anion

A

A negatively charged ion

45
Q

How to write the chemical formula for an ion

A

(Element name)+⁽ᶜʰᵃʳᵍᵉ⁾

46
Q

What’s the difference between an atom and an ion?

A

An atom has a neutral charge while an ion doesn’t.

47
Q

An ionic bond is formed between _____

A

A metal and a non-metal

48
Q

How is an ionic bond formed

A

When an atom transfers electrons to another atom to gain a full outer shell

49
Q

How to find the amounts of atoms in an ionic bond

A

Count how many of each atom is required to make an overall neutral charge

50
Q

How to name an ionic compound

A

(Metal)+(non-metal)-ide

51
Q

A covalent bond is formed between __________

A

Two or more non-metals

52
Q

How does a covalent bond work?

A

The atoms “share” electrons to create full valence shells

53
Q

What are three differences between covalent and ionic bonds

A
  • An ionic bond involves the transfer of electrons while a covalent bond involves the sharing of electrons
  • An ionic bond is between a metal and a non-metal while a covalent bond is between two non-metals
  • An Ionic bond creates ions while a covalent bond doesn’t
54
Q

What is a polyatomic ion

A

When a covalently bonded molecule creates an ionic bond with another atom to achieve a full valence shell

55
Q

What is metallic bonding

A

Where atoms of the same metal element lose their outer electrons to make a sea of delocalised electrons

56
Q

Why are metals good conductors of electricity?

A

Because the electrons are no longer bound, they can be forced to move, creating a current.

57
Q

Why are metals Malleable and Ductile?

A

The free moving electrons can slide when pressure is applied.

58
Q

Where Alkali metals are located?

A

In the Leftmost group (group 1) of the Periodic table

59
Q

Where are Alkali Earth Metals located?

A

In the second leftmost Group (group 2) on the periodic table

60
Q

Where are the Halogens located?

A

In the second rightmost group (group 17) of the periodic table

61
Q

Where are the noble gasses located?

A

In the very rightmost group (group 18) on the periodic table

62
Q

Which groups are the most reactive and why

A

Alkali metals, Alkali earth metals and Halogens. They are the most reactive because they are so close to having a full valence shell

63
Q

Which group doesn’t react and why

A

Noble gasses because they already have a full valence shell

Year 9 WCC Exam Revision (14 decks)

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